Jove
Visualize
Contact Us
JoVE
x logofacebook logolinkedin logoyoutube logo
ABOUT JoVE
OverviewLeadershipBlogJoVE Help Center
AUTHORS
Publishing ProcessEditorial BoardScope & PoliciesPeer ReviewFAQSubmit
LIBRARIANS
TestimonialsSubscriptionsAccessResourcesLibrary Advisory BoardFAQ
RESEARCH
JoVE JournalMethods CollectionsJoVE Encyclopedia of ExperimentsArchive
EDUCATION
JoVE CoreJoVE BusinessJoVE Science EducationJoVE Lab ManualFaculty Resource CenterFaculty Site
Terms & Conditions of Use
Privacy Policy
Policies

Related Concept Videos

Valence Bond Theory02:42

Valence Bond Theory

10.5K
Coordination compounds and complexes exhibit different colors, geometries, and magnetic behavior, depending on the metal atom/ion and ligands from which they are composed. In an attempt to explain the bonding and structure of coordination complexes, Linus Pauling proposed the valence bond theory, or VBT, using the concepts of hybridization and the overlapping of the atomic orbitals. According to VBT, the central metal atom or ion (Lewis acid) hybridizes to provide empty orbitals of suitable...
10.5K
Valence Bond Theory02:45

Valence Bond Theory

47.1K
Overview of Valence Bond Theory
47.1K
Ionic Bonding and Electron Transfer02:48

Ionic Bonding and Electron Transfer

47.9K
Ions are atoms or molecules bearing an electrical charge. A cation (a positive ion) forms when a neutral atom loses one or more electrons from its valence shell, and an anion (a negative ion) forms when a neutral atom gains one or more electrons in its valence shell. Compounds composed of ions are called ionic compounds (or salts), and their constituent ions are held together by ionic bonds: electrostatic forces of attraction between oppositely charged cations and anions. 
47.9K
Complexation Equilibria: Factors Influencing Stability of Complexes01:09

Complexation Equilibria: Factors Influencing Stability of Complexes

684
In complexation reactions, metal cations are the electron pair acceptors, and the ligands are the electron pair donors. The stability of the metal complexes depends primarily on the complexing ability of the central metal ion and the nature of the ligands. Generally, the complexing ability of the metal ion depends on the size and charge of the ion. As the metal ion size increases, the stability of the metal complexes decreases, provided that the valency of the metal ion and the ligands remain...
684
Molecular Orbital Theory II03:51

Molecular Orbital Theory II

25.4K
Molecular Orbital Energy Diagrams
25.4K
Bonding in Metals02:32

Bonding in Metals

51.1K
Metallic bonds are formed between two metal atoms. A simplified model to describe metallic bonding has been developed by Paul Drüde called the “Electron Sea Model”. 
51.1K

You might also read

Related Articles

Articles linked to this work by shared authors, journal, and citation graph.

Sort by
Same author

Revisiting Mitochondrial Temperature: Steady-State Heat Transfer or Non-Steady-State Dynamics?

Acta physiologica (Oxford, England)·2026
Same author

Coumarin-Augmented Thiazole Hybrids as Dual Anticancer and Antibacterial Agents.

Chemical biology & drug design·2026
Same author

Origin-Dependence of Dipole Moments of Charged Proteins: Theoretical Foundations and Implications, Revisited.

Journal of computational chemistry·2025
Same author

Vetting molecular candidates posited for the first diffuse interstellar bands (5780 and 5797 Å): a quantum chemical study.

Physical chemistry chemical physics : PCCP·2025
Same author

Electrical homeostasis of the inner mitochondrial membrane potential.

Physical biology·2025
Same author

The Analysis of Electron Densities: From Basics to Emergent Applications.

Chemical reviews·2024

Related Experiment Video

Updated: Dec 5, 2025

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
06:44

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Published on: March 24, 2018

69.4K

Bonding and metastability for Group 12 dications.

SeyedAbdolreza Sadjadi1, Chérif F Matta2,3, Ian P Hamilton4

  • 1Department of Physics, Faculty of Science, Laboratory for Space Research, The University of Hong Kong, Hong Kong SAR, China.

Journal of Computational Chemistry
|October 16, 2020
PubMed
Summary

This study investigates the electronic structure and bonding of Group 12 dications (Zn2²⁺, Cd2²⁺, Hg2²⁺), revealing their metastability using advanced quantum chemical methods. The findings highlight the Bohm quantum potential as a promising tool for understanding chemical bonding and metastability.

Keywords:
Laplacian of the electron densityOne-electron Bohm quantum potentialbonding and metastabilityclassically forbidden regions for electronsquantum theory of atoms in molecules (QTAIM)

More Related Videos

The Synthesis of [Sn10SiSiMe334]2- Using a Metastable SnI Halide Solution Synthesized via a Co-condensation Technique
12:43

The Synthesis of [Sn10SiSiMe334]2- Using a Metastable SnI Halide Solution Synthesized via a Co-condensation Technique

Published on: November 28, 2016

8.9K
Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy
07:49

Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy

Published on: February 20, 2020

9.7K

Related Experiment Videos

Last Updated: Dec 5, 2025

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding
06:44

From Molecules to Materials: Engineering New Ionic Liquid Crystals Through Halogen Bonding

Published on: March 24, 2018

69.4K
The Synthesis of [Sn10SiSiMe334]2- Using a Metastable SnI Halide Solution Synthesized via a Co-condensation Technique
12:43

The Synthesis of [Sn10SiSiMe334]2- Using a Metastable SnI Halide Solution Synthesized via a Co-condensation Technique

Published on: November 28, 2016

8.9K
Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy
07:49

Characterizing Lewis Pairs Using Titration Coupled with In Situ Infrared Spectroscopy

Published on: February 20, 2020

9.7K

Area of Science:

  • Computational Chemistry
  • Quantum Chemistry
  • Materials Science

Background:

  • Group 12 dications (M₂²⁺) exhibit unique electronic structures.
  • Characterizing the metastability of these dicationic species is crucial for understanding their stability and reactivity.
  • Traditional bonding indices may not fully capture the nuances of metastability in these systems.

Purpose of the Study:

  • To investigate the electronic structure and bonding properties of Group 12 dications (M₂²⁺, M = Zn, Cd, Hg).
  • To characterize the metastability of these species using electron density-derived quantities.
  • To explore the utility of the Bohm quantum potential and localization-delocalization matrices (LDMs) in describing bonding and metastability.

Main Methods:

  • Quantum theory of atoms in molecules (QTAIM) framework.
  • Analysis of electron density, Laplacian of electron density (∇²ρ(r)), and one-electron Bohm quantum potential (Q).
  • Calculation of localization-delocalization matrices (LDMs) and interacting quantum atoms (IQA) energies.

Main Results:

  • Estimated barriers for dissociation (BFD) for Zn₂²⁺, Cd₂²⁺, and Hg₂²⁺ range from 22.8 to 26.4 kcal/mol.
  • LDMs effectively differentiate Group 12 M₂²⁺ from isoelectronic Group 11 M₂.
  • The one-electron Bohm quantum potential shows promise in identifying regions of metastability, unlike classical bonding indices.

Conclusions:

  • Group 12 dications exhibit metastability, with quantifiable dissociation barriers.
  • The Bohm quantum potential offers a valuable perspective on chemical bonding and metastability.
  • LDMs serve as effective electronic fingerprints for distinguishing between different metallic dication systems.